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practice_final_exam - CHM-201-03 Practice Final Exam Fall...

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Unformatted text preview: CHM-201-03 Practice Final Exam Fall 2009 Page 1 of 6 CHM-201-03 Fall 2009 Professor Lin Practice Final Exam December, 2009 1.000 atm = 760 mm Hg = 760 torr = 1.013 x 105Pa = 14.7 psi; h  6.626 x 10 34 J s, c  3 × 108 m/s R = 0.08206 L • atm mol • K Atomic Weights (amu) H 1.008 He 4.00 C 12.01 Ar 39.95 Ne 20.18 NA = 6.022 x 1023molecules or atoms/mole Molecular Weights (amu or g/mol) 44.01 CO2 44.02 N2O 92.02 N2O4 46.01 NO2 2.02 H2 K = oC + 273 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) All of the following are properties of sodium. Which one is a physical property of sodium? ( A) It is surface turns black when first exposed to air. B) It is a solid at 25°C and changes to a liquid when heated to 98°C. C) When placed in water it sizzles and a gas is formed. D) When placed in contact with chlorine it forms a compound that melts at 801°C. E) Sodium is never found as the pure metal in nature. 2) The SI prefixes milli and mega represent, respectively: D) 10–3 and 109. A) 106 and 10–6. –3 6 E) 10–6 and 10–3. B) 10 and 10 . C) 103 and 10–6. 3) Lead melts at 601.0°C. What temperature is this in °F? A) 302°F B) 365°F C) 1,050°F ) D) 1,082°F E) 1,114°F 4) One of the common intravenous fluids, called physiological saline, is a homogeneous mixture of NaCl in water. In this mixture, 0.89% of the mass is contributed by the NaCl. What mass of NaCl is found in 450. mL of physiological saline? (Given: density of physiological saline = 1.005 g/cm3) A) 2.0 g B) 4.0 g C) 5.1 g D) 508 g E) 400 g 5) Based on the solubility rules, which of the following will occur when solutions of ZnSO4(aq) and MgCl2(aq) are mixed? A) ZnCl2 will precipitate; Mg2+ and SO42– will be spectator ions. B) ZnSO4 will precipitate; Mg2+ and Cl– will be spectator ions. C) MgSO4 will precipitate; Zn2+ and Cl– will be spectator ions. D) MgCl2 will precipitate; Zn2+ and SO42– will be spectator ions. E) No precipitate will form. CHM-201-03 Practice Final Exam Fall 2009 6) The general electron configuration for atoms of all elements in Group 5A is B) ns2np5 C) ns2np4 D) ns2np3 E) ns2np1 A) ns2np6 Page 2 of 6 7) What mass of K2CO3 is needed to prepare 200. mL of a solution having a potassium ion concentration of 0.150 M? A) 4.15 g B) 10.4 g C) 13.8 g D) 2.07 g E) 1.49 g 8) The oxidation number of Cr in Cr2O72– is A) –12 B) –7 C) –2 . D) +6 E) +7 9) Which one of the following is a redox reaction? A) 2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g) B) 2KBr(aq) + Pb(NO3)2(aq) → 2KNO3(aq) + PbBr2(s) C) CaBr2(aq) + H2SO4(aq) → CaSO4(s) + 2HBr(g) D) H+(aq) + OH– (aq) → H2O(l) E) CO32– (aq) + HSO4–(aq) → HCO3– (aq) + SO42– (aq) 10) Octane (C8H18) undergoes combustion according to the following thermochemical equation: ∆H°rxn = –11,020 kJ/mol. 2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(l) Given that ∆H°f[CO2(g)] = –393.5 kJ/mol and ∆H°f[H2O(l)] = –285.8 kJ/mol, calculate the standard enthalpy of formation of octane. A)–210 kJ/mol B)–11,230 kJ/mol C)22,040 kJ/mol D)–420 kJ/mol E)420 kJ/mol 11) For which of the following reactions is the enthalpy change equal to the second ionization energy of nitrogen? D) N–(g) + e– → N2–(g) A) N2+(g) → N3+(g) + e– E) N+(g) → N2+(g) + e– B) N2+(g) + e– → N+(g) 2+ – C) N(g) → N (g) + 2e 12) Which of the following compounds is a weak electrolyte? C) C6H12O6 (glucose) D) N2 A) HCl B) NH3 13) Transition metal elements have atoms or ions with partially filled A) s subshells. B) p subshells. C) d subshells. D) f subshells. 14) Which of the following make an isoelectronic pair: Cl–, O2–, F, Ca2+, Fe3+? B) O2– and F C) F and Cl– D) Cl– and Ca2+ A) Ca2+ and Fe3+ 15) How many unpaired electrons are there in an F ion? A) 0 B) 1 C) 2 D) 3 E) KCl E) g subshells. E) None of the above. ( ) E) This cannot be predicted. 16) Which of the following elements behaves chemically similarly to oxygen? A) magnesium B) sodium C) sulfur D) chlorine E) iron F) beryllium CHM-201-03 Practice Final Exam Fall 2009 Page 3 of 6 17) Complete and balance the following redox equation. When properly balanced using the smallest whole-number coefficients, the coefficient of S is H2S + HNO3 → S + NO (acidic solution) A) 1 B) 2 C) 3 D) 5 E) 6 18) Which of the following elements has the smallest first ionization energy? A) Cl B) Na C) Be D) K E) As 19) After carrying out the following operations, how many significant figures are appropriate to show in the result? (13.7 + 0.027) ÷ 8.221 A) 1 B) 2 C) 3 D) 4 E) 5 20) Based on the solubility rules, which one of the following compounds should be insoluble in water? C) FeCl2 D) AgBr E) ZnCl2 A) NaCl B) MgBr2 21) Which of the following elements has the greatest electron affinity (largest positive value)? A) K B) Br C) As D) Ar E) I 22) The second ionization energy of Mg is ________ than its first ionization energy, and is __________ than the second ionization energy of Na. A) higher, higher B) lower, higher C) higher, lower D) lower, lower SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question. 23) a. What is the standard enthalpy of formation of H2(g) at 25°C? b. What is the ground-state electron configuration for chlorine? c. What is the total number of electrons possible in the 2p orbitals? 24) (4 pts) a. If we take away two electrons from the outer shell of calcium, it would have the same electron configuration as what element? b. The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of these colors, _______ has the most energy. 25) (4 pts) a. Give an example of an extensive property. b. Give an example of an intensive property. c. Name the following compounds: FeSO4 Mg(NO3)2 CuBr2 CS2 CHM-201-03 Practice Final Exam Fall 2009 26) a. Which of the following molecules should be polar? a. CH3OH b. H2O c. CH3OCH3 Page 4 of 6 b. Write a Lewis structure for the chlorate ion, ClO3–, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for ClO3– that obey the octet rule. c. N,N-diethyl-m-tolumide (DEET) is the active ingredient in many mosquito repellents. How many sigma bonds and pi bonds are contained in a DEET molecule? 27) (True or False) a. In an endothermic process, heat is absorbed by the system. b. Sodium ions are more reactive than sodium atoms. ( ( ) ) c. Pi bonds are covalent bonds in which the electron density is concentrated above and below a plane containing the nuclei of the bonding atoms. ( d. A weak acid or a weak base ionizes completely. e. The following equation is an example of a net ionic equation. Na+(aq) + Br–(aq) + Ag+(aq) + NO3–(aq) → AgBr(s) + Na+(aq) + NO3–(aq) ( ) ) Calculations: Show as much work as possible for partial credit. All answers should have a number AND a unit. 28) What volume of concentrated nitric acid (15.0 M) is required to make 100. mL of a 3.0 M nitric acid solution? 29) Find ∆H°rxn for the reaction 2Ag2S(s) + 2H2O(l) → 4Ag(s) + 2H2S(g) + O2(g). [∆H°f (Ag2S(s)) = –32.6 kJ/mol; ∆H°f (H2S(g)) = –20.5 kJ/mol; ∆H°f (H2O(l)) = –285.5 kJ/mol] CHM-201-03 Practice Final Exam Fall 2009 30) Calculate the energy of a photon of light with a wavelength of 360 nm. Page 5 of 6 31) Classify the following as a physical or chemical change: a. Food spoils; b. Newspaper burns. 32) Complete the following table. Hybrid type a ___________ b sp3 c s p2 Geometry of electron pairs linear _________ __________ 33) Given the following ∆H° values, H2(g) + 1 2 O2(g) → H2O(l) ∆H°f = –285.8 kJ/mol H2O2(l) → H2(g) + O2(g) ∆H°rxn = 187.6 kJ/mol calculate ∆H°rxn for the reaction H2O2(l) → H2O(l) + 1 2 O2(g), 34) (4 pts) What is the mass of 1.00 dm3 of mercury in kg? The density of mercury is 13.6 g/cm3. 35) (4 pts) At STP, 1 mole of gas has a molar volume of 22.4 L. What is the density of oxygen at STP? 36) Ferrocene, Fe(C5H5)2(s), can be prepared by reacting 3.0 g of FeCl2(s) with an equal mass of cyclopentadiene, C5H6(l), and an excess of KOH, as shown in the following reaction FeCl2 + C5H6 + KOH → FeC10H10 + H2O A. Balance the chemical equation. B. What is the limiting reagent in this procedure? C. Based on your answer to part A, what mass of Fe(C5H5)2 could theoretically be formed? CHM-201-03 Fall 2009 1. B 2. B 3. E 4. B 5. E 6. D 7. D 8. D Practice Final Exam Answer Key December, 2009 CHM-201-03 Practice Final Exam Fall 2009 Page 6 of 6 9. A 10. A 11. E 12. B 13. C 14. D 15. A 16. C 17. C 18. D 19. C 20. D 21. B 22. C 23. a. 0 kJ/mol; b. 1s22s22p63s23p5 or [Ne]3s23p5; c. 6. 24. a. argon; b. violet. 25. a. Mass, length, and volume; b. Temperature, density, melting point, boiling point; c. iron(II) sulfate; copper(II) bromide; magnesium nitrate; carbon disulfide. 26. a. All of these are polar molecules; b. Total number of resonance structures of this type (that obey the octet rule) = 3. c. 31 sigma bonds and 4 pi bonds. 27. a. True; b. False; c. True; d. False; e. False. 28. 20. mL. 29. 595.2 kJ/mol. 30. 5.5 × 10 –19 J. 31. a. chemical; b. chemical. 32. Geometry of electron pairs Hybrid type a sp linear tetrahedral b sp3 2 trigonal planar c sp 33. –98.2 kJ/mol. 34. 13.6 kg. 35. 1.43 g/L 36. A. FeCl2 + 2C5H6 + 2KOH → FeC10H10 + 2H2O B. C5H6 is limiting C. 4.2 g of ferrocene . ...
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This note was uploaded on 02/10/2011 for the course CHEM 201 taught by Professor Griffen during the Fall '09 term at Bunker Hill.

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